
When diluting the commercial vinegar, what would have been the effect on acetic acid molairty of failing to rinse the pooped with commercial vinegar, assuming there was some distilled water left in the piper from a previous student? ( think about how the

Acetic acid (HC2H3O2) is an important component of vinegar. A 10.00mL sample of vinegar is titrated with .5052 M NaOH, and 16.88 mL are required to neutralize the acetic acid that is present. a.write a balanced equation for this neutralization reaction

1. Commercial vinegar is a solution of acetic acid in water. How would you determine which brand of vinegar contains more acetic acid in a given volume of vinegar?

The cafeteria decides to save money by using concentrated acetic acid (CH3COOH at 17.5 mol/L) and diluting it with water toproduce vinegar (5.00% m/v aceticacid). a) What is the concentration of vinegar in mol/L?b) What volume of vinegar can the cafeteria

The cafeteria decides to save money by using concentrated acetic acid (CH3COOH at 17.5 mol/L) and diluting it with water toproduce vinegar (5.00% m/v aceticacid). a) What is the concentration of vinegar in mol/L?b) What volume of vinegar can the cafeteria


10 ml sample of vinegar an aqueous solution 0f acetic acid( HC2H3O2) is titrated with 0.5062 M and 16.58 ml is required to reach equivalence point what is the molarity of the acetic acid b. if the density of vinegar is 1.006 g/cm3 what is the mass percent

A 10.0 mL of vinegar, an aqueous solution of acetic acid (HC2H3O2), is titrated with .5062M NaOH, and 16.58mL is required to reach the equivalence point. A. What is the molarity of the acetic acid? B. If the density of the vinegar is 1.006 g/cm^3, what is

AcidBase Titrations a) How will the concentration of NaOH be affected if during the titration some of the solid potassium hydrogen phthalate was spilled during the transfer? Will the concentration of the standardized NaOH increase, decrease, or have no

Could you help me find some websites that can tell me what the ingredients are in vinegar. http://en.wikipedia.org/wiki/Vinegar Vinegar is acetic acid. Some bottles are sold as 4% and some as 5%. White vinegar is straight acetic acid (distilled) and water.

a) How will the concentration of NaOH be affected if during the titration some of the solid potassium hydrogen phthalate was spilled during the transfer? Will the concentration of the standardized NaOH increase, decrease, or have no effect? b) How will the

a) How will the concentration of NaOH be affected if during the titration some of the solid potassium hydrogen phthalate was spilled during the transfer? Will the concentration of the standardized NaOH increase, decrease, or have no effect? b) How will the

We did a titration lab, and one of the postlab questions says: "the manufacturer of the vinegar used in this experiment claims that the vinegar contains 5% acetic acid by weight. Use your results and a density of 1g/mL to determine if this claim is true

We did a titration lab, and one of the postlab questions says: "the manufacturer of the vinegar used in this experiment claims that the vinegar contains 5% acetic acid by weight. Use your results and a density of 1g/mL to determine if this claim is true

In this experiment NaOH is standardized to find out the percent by mass of the acetic acid in a sample of vinegar. A student had not allowed the NaOH pellets to dissolve completely before standardizing it with KHP, but when the student refilled the buret

what is the theoretical value for the M of acetic acid in vinegar if the vinegar is 5% acetic acid by a % mass value. Additional info: the experimental M of the acetic acid in vinegar is 0.80M Thank you!!


what is the theoretical value for the M of acetic acid in vinegar if the vinegar is 5% acetic acid by a % mass value. Additional info: the experimental M of the acetic acid in vinegar is 0.80M Thank you!!

Vinegar is a solution of acetic acid, CH3COOH, dissolved in water. A 4.69 g sample of vinegar was neutralized by 32.97 mL of 0.100 M NaOH. What is the percent by weight of acetic acid in the vinegar?

Vinegar is 5% acetic acid. If the density of household vinegar is approximately 1.00 g/mL, how many grams of acetic acid are contained in 10.0 mL of vinegar? So I started out with 10.0 mL of HC2H3O2 then multiplied by 1.00g/1mL. What do I do next? Is it

If acetic acid is the only acid that vinegar contains [Ka = 1.8*105] , calculate the concentration of acetic acid in the vinegar. pH of vinegar is 3.20 _______________ First I got the antilog of the pH given, which turned out to be 6.309E4. Then I did

Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if

4. Vinegar is a dilute solution of acetic acid. What is the concentration of acetic acid in the vinegar if 26.5 mL of NaOH at 0.250 M are required to neutralize 10.0 mL of vinegar?

Vinegar is a dilute solution of acetic acid. What is the concentration of acetic acid in the vinegar if 26.5 mL of NaOH at 0.250 M are required to neutralize 10.0 mL of vinegar?

Acetic acid, HC2H3O2, is the sour constituent of vinegar (acetum is Latin for "vinegar" ). In an experiment, 3.76 g of acetic acid was burned. HC2H3O2(l) + 2 O2(g) 2 CO2(g) + 2 H2O(l) If 54.6 kJ of heat evolved, what is ÄH per mole of acetic acid?

Calculate the mole fraction of acetic acid in vinegar, assuming that vinegar is 5.00% acetic acid(by mass) and that the density of vinegar is 1.05 g/mL

Hi, could someone help me with these calculations for my lab; Given: Volume of vinegar analyzed:5 mL Con'c of NaOH: 0.09890M Avg. V of NaOH from titration:43.75 mL Moles of NaOH required to reach the equivalence point: ? Would this be


In a crazy scenario, the Oylan Vinegar Company has 10,000 gallons of vinegar with 0.622% concentration. This vinegar solution cannot be sold because it's too weak, but the plant manager can't bear to discard it. OVC also has a large batch of vinegar that

Ok, in this question, the drops is throwing me off totally, can someone help! A nationally known company markets a product called "cleaning vinegar" that is not designed for human consumption. What is the mass percent of acetic acid in this product if 25

A chemist wants to be a supercook and wants to create 8%(m/v) acetic acud solution to be "extra strength" vinegar. if pure acetic acid Is a liquid density of 1.049 g/ml. how many ml of acetic acid should be dissolved to male 500 ml of 8% acetic acid?

Thanks for your help; I am still have a few problems, could you check my work: Given: Volume of vinegar analyzed5mL Con'c of NaOH0.09890M Avg. Volume of NaOH from titration43.75mL Density CH3COOH: 1.049g/mL Calculations: 1.Moles of NaOH required to

Assuming that the lab procedure was conducted in an identical manner in all other respects, if a large quantity of vinegar had been taken initially for analysis, for example, a 50.0 ml instead of 25.0mL discuss briefly how each of the following would

vinegar is 5.0% acetic acid, CH3COOH, by mass. vinegar has a density of 1.02 g/ml what is the madd of acetic acid in 50.0 ml of vinegar?

A 5.00 mL aliquot of vinegar (acetic acid, FW = 63 g/mol) was diluted and titrated with 0.1104 M NaOH requiring 32.88 mL. If the vinegar has a density of 1.055 g/mL, calculate its acidity as % acetic acid

Assuming that the lab procedure was conducted in an identical manner in all other respects, if a large quantity of vinegar had been taken initially for analysis, for example, a 50.0mL instead of 25.0 mL discuss briefly how each of the following would

a 10 ml vinegar sample was completely neutralized by 22.5 0.2M NaOH solution . calculate the molarity and percent acetic acid in vinegar I keep getting 2.7% acetic acid is this correct? my friend got 27% and if I am wrong where do you think I messed up?

Assuming the density of vinegar is 1.0 g/mL ' what is the molarity of vinegar? (use the percent by mass of acetic acid to vinegar which is 5%.) The molar mass of acetic acid is 60.05 g/mol?


To titrate the acetic acid in 10.0 mL of vinegar sample, 25.5mL of 0.5M sodium hydroxide solution is needed. What is the concentration of acetic acid in the vinegar?

A vinegar sample is found to have a density of 1.006 {\rm{ g/mL}} and to contain 4.2\% acetic acid by mass.How many grams of acetic acid are present in 1.20L of this vinegar?

A vinegar sample is found to have a density of 1.006 and to contain 4.7 acetic acid by mass.How many grams of acetic acid are present in 3.00 of this vinegar?

A chemist wants to be a supercook and wants to create 8%(m/v) acetic acud solution to be "extra strength" vinegar. if pure acetic acid Is a liquid density of 1.049 g/ml. how many ml of acetic acid should be dissolved to male 500 ml of 8% acetic acid? It

assuming the vinegar solution has a density of 1.01 g/mL, calculate the percent by weight of actic acid (CH3CO2H) in your sample of vinegar. How does the value compare with 5% the value for the % acetic acid in normal vinegar? Thanks!

Vinegar is a 5.0% solution by weight of acetic acid in water. Given that the pH for vinegar is 2.41 and that Ka= 1.8E5 and the density s 1.00g/mL, what is the percent dissociation of acetic acid in vinegar? I know the % dissociation equals the amount

Could someone help me with this question? A vinegar sample was analyzed and found to be 5.88% acetic acid by volume. The density of pure acetic acid is 1.409g/ml. What volume of 0.200 M NaOH would be required to titrate a 2 ml aliquot of this vinegar.

I want to know HOW to do the problems, not just an answer please. 1.) How many moles of ions are released when 0.27 moles of CoCl2 is dissolved in water? 2.) A 5.54g sample of vinegar was neutralized by 30.10 mL of 0.100M NaOh. What is the precent (by

A vinegar sample was analyzed and found to be 5.88% acetic acid by volume. The density of pure acetic acid is 1.049g/mL. What volume of 0.200M NaOH would be required to titrate a 2ml aliquot of this vinegar? Some help would be greatly appreciated! thanks

which has the most acid coke or vinegar I don't have any numbers to support my thinking but I know MOST brands of vinegar are 5% acetic acid (although I saw one recently at 4%). I think coke is about 0.05 M but I don't KNOW that. In addition, k1 for H2CO3


hi, I am trying to find the solubility of Sodium Acetate by using 0.100 mol Hydroxide(base) and 0.837 mol acetic acid( vinegar). The theoretical solubility of sodium acetate is 82.3g/100ml at 25C. Doing calculations we would want NAOH concentration of

I need help please. The question is vinegar, or a dilute of CH3COOH (acetic acid), should have a molarity of around 0.83 M. Using the Ka for acetic acid, what should the pH of vinegar be?? Thank you!!

Trying to find mass percent of acetic acid in 25 drops of .683M NaOH solution are required to neutralize 10 drops of cleaning vinegar. Assume that the density of the cleaning vinegar is the same as the density of regular vinegar which is 1.05 g ml1 You

Using the data collected for part c on your data sheet and assuming the density of the vinegar is 1.00g/mL, 1) calculate the molar concentration of acetic acid (CH3COOH) in the vinegar sample using the average volume of NaOH. 2) calculate the mass percent

Using the data collected for part c on your data sheet and assuming the density of the vinegar is 1.00g/mL, 1) calculate the molar concentration of acetic acid (CH3COOH) in the vinegar sample using the average volume of NaOH. 2) calculate the mass percent

Greetings: I was wondering how to calculate the weight/volume % of vinegar using the formula w/v Per Cent = g/100 mL or grams per deciliter: WHAT WEIGHT DO I USE NaOH, Acetic ACID? the data include: volume of NaOH needed to neutralize

Help! I need to do this review question and don't know where to start ! The label on a bottle of vinegar claims that the bottle conatins 5% (m/v) of acetic acid. In order to test this claim, a 50ml sample is titrated with sodium hydroxide. 166ml of 0.25

vinegar is 5% acetic acid by mass and has a density of 1.02g/mL.what mass of acetic acid ,in grams, is present in 185 mL of vinegar.

If acetic acid is the only acid that vinegar contains , calculate the concentration of acetic acid in the vinegar. if the pH of vinegar is 2.7

hi, I am trying to find the solubility of Sodium Acetate by using 0.100 mol Hydroxide(base) and 0.837 mol acetic acid( vinegar). The theoretical solubility of sodium acetate is 82.3g/100ml at 25C. Doing calculations we would want NAOH concentration of


why would acetic acid concentration of a good vinegar need to be known for commercial reasons and regulatory health and safety reasons

Commercial vinegar usually has a concentration of 5%, per volume. a) Calculate the [H3O+] , if the density of acetic acid is 1.051 g/mL. b) Calculate the pH.

Calculate the pH of a solution that obtained by diluting 0.015 mol acetic acid with water to 250 cm3 (the Ka  value for acetic acid is 1.74 x 105 M).

100.0 mL Vinegar (d=1.06g/mL) contains 4% acetic acid. a. How many moles of acid are in 100 mL of vinegar? b. How many mL of 0.11 M NaOH are required to neutralize the vinegar?

A solution of vinegar is 5.16% by mass aetic acid, CH3CO2H, in water. Assuming the density of vinegar is 1.00 g/mL, what is the molarity of the acetic acid?

A 12.6 mL sample of vinegar, containing acetic acid, was titrated using 0.542 M NaOH solution. The titration required 24.1 mL of the base. what is the molar concentration of acid in the vinegar?'

A certain vinegar is 5.0% acetic acid in water. What mass (in grams) of acetic acid is needed to mix with 185 grams of water to prepare this vinegar?

Vinegar is a dilute solution of acetic acid. In the titration of 5.00 mL of vinegar, 39.75 mL of 0.137 M sodium hydroxide solution was required to neutralize the vinegar to a phenolphthalein end point. Calculate each of the following of the vinegar. (a)

This soidum hydroxide solution was then used to determine the amount of acetic acid in vinegar. Three titrations of the sodium hydroxide solution against exactly 5mL of vinegar using phenolphthalein indicator required 22.85Ml, 22.67mL and 22.93mL of the

vinegar is made by adding 33 g of acetic acid to 625 if water what is the percent by mass of acetic acid in this solution of vinigar


If i have the cost per quart of vinegar and the % of acetic acid for each of 4 brands, what would be an equation i could use to find out which brand has the most acetic acid for the money?

A vinegar contains acetic acid, CH3COOH. Titration of 5.000g of vinegar with 0.100, NaOH requires 33.0 ml to reach equivalent point. What is the weight percentage of CH3COOH in vinegar?

If a 11.0 mL sample of vinegar (aqueous acetic acid ) requires 19.0 mL of 0.500 M NaOH to reach the endpoint, what is the original molarity of the acetic acid solution?

a vinegar contains acetic acid,CH3COOH.Titration of 5.00g of vinegar with 0.100M of NAOH requires 33.00cm to reach the equivalence point.a)what is the weight percentage of CH3COOH in vinegar?

Is this balanced properly 2H2O2> 2H2O +O2 Thank you for the reactions of zinc and acetic acid. REAL QUESTION, if I was to rub all the copper off of a new penny down to the zinc, what would be the appearance of the zinc if I left it in vinegar (acetic

Please tell me if these are right! 1.How many milliliters of 0.215 M NaOH solution are needed to completely neutralize 2.50 ml of 0.825 M H2SO4 solution? I got 19.2 ml 2. A 10.0ml sample of vinegar which is an aqueous solution of acetic acid HC2G3O2

When you mixand separate CaCO3 and SiO2 with acetic acidvinegar, it is a chemical reaction. It bubbles and CO2 is produced. What property of CaCO3 causes this to happen? Could you explain this to me pls. I am guessing the acetic acid reacts with one of

The data below was collected while performing a titration of acetic acid (in vinegar) to determine its concentration using sodium hydroxide. 150 ml of vinegar with unknown molarity 45.5 ml of .5 M NaOH was added to reach equivalence point Find the molarity

My mind is bleeding again. I am trying to figure out the molarity of acetic acid in Vinegar. We used a standard solution of .613 Molars of NaOH. We added 33.75mL of NaOH to completely titrate/neutralize 25mL of Vinegar and we're supposed to be able to

If you assume that there is 5% acetic acid in vinegar, how much vinegar should you weigh out so that the endpoint requires 25.0 mL of 0.186 M NaOH?


The volume of acetic acid in a sample of 500mL of vinegar is determined to be 1mL. What is the v/v percentage of the vinegar?

1 the vinegar soltion sold in the store is about 5% acetic acid. Assuming that the solution has a density of 1.01 g/mL, calculate the pH of vinegar.

3.30 mL of vinegar needs 43.0 mL of 0.150 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.70 qt sample of this vinegar?

If 3.30 mL of vinegar needs 42.5 mL of 0.150 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.50 qt sample of this vinegar?

If 3.15 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.40 qt sample of this vinegar?

How much vinegar at 5% acetic acid concentration would be required to neutralize 100mL of 0.01 M NaOH? (Assume a density of vinegar to be 1.01g/mL)

Given that the density of the supplied vinegar solution in this experiment is 1.025 g/mL, calculate the % acetic acid found in the vinegar sample.

3.30 mL of vinegar needs 40.0 mL of 0.150M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.10 qt sample of this vinegar?

given that thee density of a supplied vinegar solution in an experiment is 1.025g/ml, what is the percentage acetic acid found in the vinegar sample?

a 10.0mL vinegar sample was completely neutralized by 22.5mL 0.2M NaOH solution. calculate molarity and % of acetic acid in vinegar. please help


I'm doing a vinegar titration lab and i need to know how can my acetic acid in vinegar be affected if a few droops of NaOH solution is not washed down with distilled water

A total of 31.3 ml of 0.15 N NaOH was required to reach a phenolphthalein endpoint in titrating 6.00 g of vinegar. Calculate the number of equivalents of acetic acid in vinegar.

A total of 31.3 ml of 0.15 N NaOH was required to reach a phenolphthalein endpoint in titrating 6.00 g of vinegar. Calculate the number of equivalents of acetic acid in vinegar.

calculating the molarity of acetic acid in a vinegar sample given that 5.00 of vinegar required 43.50 mL of 0.1050 M NaOH to just reach the methyl red endpoint.

Vinegar is a solution of acetic acid, a weak acid. How can you produce more acetate ions in the solution? CH 'subtext' 3 COOH(aq) H+(aq) + CH 'subtext' 3 COO^ (aq) A. Evaporate some of the water. B. Decrease the pressure. C. Increase the volume of the

A 30.84 mL volume of 0.128 M NaOH is required to reach the phnolphthalein endpoint in the titration of a 5.441 g sample of vinegar. Calculate % acetic acid in the vinegar.

A 31.43 mL volume of 0.108 M NaOH is required to reach the phnolphthalein endpoint in the titration of a 4.441 g sample of vinegar. Calculate % acetic acid in the vinegar.

Please help me... I don't understand this at all. I need to calculate the molarity of the acetic acid in this problem: A 4,00 mL sample of vinegar (acetic acid) was tirated with 0.1250M NAOH according to the following equation: HC2H3)s + NAOH  NAC2H3O2

calculate the molarity of acetic acid in a vinegar sample,knowing that 5.00ml of vinegar requires 43.50ml of 0.105 M NaOH to just reach the phenolphthalein endpoint in a titration

calculate the molarity of acetic acid in a vinegar sample,knowing that 5.00ml of vinegar requires 43.50ml of 0.105 M NaOH to just reach the phenolphthalein endpoint in a titration


A 10.0mL sample of vinegar, which is an aqueous solution of acetic acid, CH3COOH, requires 16.5 XML of a 0.500M NaOH solution to reach the endpoint in a titration (where the moles of acid are equal to the moles of base). What is the molarity of the acetic

A 10.0 ml sample of vinegar which is an aqueous solution of acetic acid, requires 16.5ml of a 0.500M NaOH solution to reach the endpoint in a titration (where the moles of acid are equal to the moles of base). What is the molarity of the acetic acid

I did a lab on vinegar and titration. The question asks.. In the titration of acetic acid and NaOH the use of the color indicator mandates that excess base be present to detect the reading endpoint. Will this cause the calculated and reported mass percent

For a lab, I have to write out the balanced equation for the titration of vinegar (containing acetic acid) with sodium hydroxide. But I am unsure of how to split up vinegar... CH3COOH + NaOH > ? I need help writing out the products... Lucy

Titration was used to determine the molarity of acetic acid in vinegar. A primary standard solution of KHP was used to standardize the NaOH. 1. When performing this experiment, impure KHP was used to standardize the NaOH solution. If the impurity is